Amphee

The initial pressure for the compounds involved in the reaction shown were determined to be P(Br2(g)) = 0.5417 atm, P(Cl2(g)) = 0.6962 atm, P(BrCl(g)) = 0.3442 atm. Calculate the value of the equilibrium constant (Kp) at 1000 K if the equilibrium pressure...

If the initial concentration of NO(g) is 6.745 mol/L, calculate the % of NO(g) left over after the reaction reaches equilibrium according to the balanced equation. The value of Kc at 2400 K is 400.00. The initial concentration of the reaction products is...

The value of the equilibrium constant (Kp) as represented by the first chemical equation is 1.02 x 102 at 727 °C. Calculate the value of the equilibrium constant (Kp) for the second equation at the same temperature. Express answer in scientific notation....

When a sample of NO2(g) (849.9 grams) is placed in 390.0 L reaction vessel at 961.0 K and allowed to come to equilibrium the mixture contains 248.2 grams of NO(g). What is the concentration (mol/L) of NO2(g)? 2NO2(g) = 2NO(g)+O2(g) I keep getting .0212 or...

Pure phosgene gas (COCl2), .03mole, was placed in a 1.5 L container. It was heated to 800k, and at equilibrium the pressure of CO was found to be .497 atm. Calculate the equilibrium constant Kp for the reaction CO(g) + Cl2(g) = COCL2(g)

Consider the following equilibrium process at 686 C C02(g)+H2(g)=CO(g)+H20(g) The equilibrium concentration of the reacting species are [CO]=0.050M, [H2]=0.045M, [CO2]=0.086M, and [H20]=0.040M. (a)Calculate the Kc for the reaction at 686 C. (b) If we add...

What is the pH of the solution created by combining 12.20 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? mL NaOH pH w/HCl pH w/HC2H3O2 12.20 =================================== my work: 0.000420 moles...

9.50mL of .100M NaOH + 8.00mL of .100M of HC2H3O2. Find the pH. Okey this is what I did. 8.00-9.50=1.5mL or .0015L .0015L x .1000 = .00015 moles .00015/(total volume) = .0085714 M -log(.0085714)= 2.0669=pOH 14-2.0669 = 11.933 But I'm getting the feeling t...

At a particular temperature, k=1.6x10^-5 for the reaction 2SO3(g)=2SO2(g)+ O2 If 4 mole of SO2 and 2 mole of O2 are placed into a 2.0 L flask, calculate the equilibrium concentration of all the species. Thanks.

Thanks drbob, I was just getting confused by the direction of the equilibrium. how can you tell which way the equilibrium shifts?

Wait never mind I figured it out. 1/F = F so 1/102 right?

I got C). 33.75 or 33.8. Use Spectrometry. You have 45.0ml of NO2 right. Convert that to Liters so you get .045L. Since its at STP convert .045L to moles using 22.4 L/mol. (.002 moles of NO2)[(6 moles of NH3)/(8 moles of NO2)] = .0015 mole of NH3 use 22.4...

Thanks Dr.Bob

Never mind I got it. I was just not seeing the PV=nRT relationship here lol. Thanks anyways.

Oh yes it is a typo my bad. But you got the right answer though. Thank you and thank you for the short cut on the calculator too, I was doing it just like you did it but my the calculator was having overflow problem

HI again Dr.Bob This is what I'm doing .10M (.0122L)= .00122 moles of NaOH .00122/(.008+.0122)= .06039M .10M (.008)= .0008 moles CH3COOH .0008-.00122=.00042 moles HCl unreacted .00042/(.008+.0122)=.020792M CH3COOH pH= pka + log (x/y) pH= 4.75 + log (.0603...

Soo...what am I doing wrong? Sorry I'm a bit confused here. pH= 4.75 + log (.06040/.02079) ? Then I get 5.203 which isn't the right answer either.

THANKS DR.BOB

Never mind I figured it out. I was forgetting to make the reaction 100% to the reactant side and then working it out from there.